Challenge Review
Supplemental Instruction
Iowa State University / Leader: / Kia
Course: / CHEM 177
Instructor: / Kingston
Date: / October 27th, 2016

Lecture review

  1. Using Slater’s rule calculate the amount of a valence electron in fluorine will be shielded. (n=0.35, n-1=.85, n-2 and on =1)

5.2

  1. List at least 3 characteristics of the following
  2. Metals

Shiny luster, various colors (often silvery), solids, ductile, malleable, good conductors of heat and electricity, form cations in solns

  1. Nonmetals

No luster, various colors, solids usually brittle (some hard, some soft), poor conductors, form anions in solns

  1. Predict the products given the reactants and balance the equation
  2. 2 K(s) + 2 H2O(l)2KOH(aq) + H2(g)
  1. __ Ca(s) + 2 HCl(aq)H2(g) + CaCl2(aq)
  1. __ P4O10 + 6 H2O(l) 4 H3PO4(aq)
  1. Define the following
  2. Electron Affinity

Change in energy when an electron is added to gaseous atom

  1. Ionization Energy

Energy required to remove an electron

  1. Z-effective

Attractive force from nucleus felt by outer most electron

Group challenge questions

  1. The element bismuth (Bi, atomic number 83) is the heaviest member of group 5A. A salt of the element, bismuth subsalicylate, is the active ingredient in Pepto-Bismol, an over the counter medication for gastric distress.
  2. What accounts for the general increase in atomic radius going down the group 5A elements?
  1. Bi2O3 is a basic oxide. Write a balanced chemical equation for its reaction with dilute nitric acid. If 6.77 g of Bi2O3 is dissolved in dilute acidic solution to make 0.500 L of solution, what is the molarity of the solution of Bi3+ ion?
  1. The density of Bi at 25 degrees C is 9.808 g/cm3. How many Bi atoms are present in a cube of the element that is 5.00 cm on each edge? How many moles of the element are present?
  1. Trinitroglycerin, C3H5N3O9 (usually referred to simply as nitroglycerine), has been widely used as an explosive. Alfred Nobel used it to make dynamite in 1866. Rather surprisingly, it also is used as a medication, to relieve angina (chest pains resulting from partially blocked arteries to the heart) by dilating the blood vessels. At 1 atm pressure and 25 degrees C, the enthalpy of decomposition of trinitroglycerin to form nitrogen gas, carbon dioxide gas, liquid water, and oxygen gas is -1541.4 kJ/mol.
  2. Write the balanced chemical equation for the decomposition of trinitroglycerin.
  1. Calculate the standard heat of formation of trinitroglycerin. Standard heat of formation of CO2 and water are -393.5 kJ and -285.8 kJ respectively.
  1. A standard dose of trinitroglycerin for relief of angina is 0.60 mg. If the sample is eventually oxidized in the body to nitrogen gas, carbon dioxide gas, and liquid water, what number of calories is released?
  1. A sample of 70.5 mg of potassium phosphate is added to 15.0 mL of 0.050 M silver nitrate, resulting in the formation of a precipitate.
  2. Write the molecular equation for the reaction
  1. What is the limiting reactant in the reaction?
  1. Calculate the theoretical yield, in grams, of the precipitate that forms.
  1. The quantity of Cl- in a municipal water supply is determined by titrating the sample with Ag+. The precipitation reaction taking place during the titration forms AgCl(s). The end point in this type of titration is marked by a change in color of a special type of indicator.
  2. How many grams of chloride ion are in the sample of water if 20.2 mL of 0.100 M Ag+ is needed to react with all the chloride in the sample?
  1. If the sample has a mass of 10.0 g, what percentage of Cl- does it contain?